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18 Nov 2019
Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25 degree C. (The equation is balanced.) 3 CI_2(g) + 2 Fe(s) rightarrow 6 Cl^-(aq) + 2 Fe^3+(aq) CI_2(g) + 2 e^- righrarrow 2 CI^-(aq) E degree = +1.36 V Fe^3+(aq) + 3 e^- rightarrow Fe(s) E degree = -0.04 V A) +1.40 V B) -1.32 V C) +1.32 V D) +4.16 V E) -1.40 V Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 degree C. Sn(s)|Sn^2+(aq) 1.8 M) ||Ag^+(aq, 0.055 M)| Ag(s) A) -0.85 V B) -0.94 V C) +0.86 V D) +1.02 V E) +0.98 V
Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25 degree C. (The equation is balanced.) 3 CI_2(g) + 2 Fe(s) rightarrow 6 Cl^-(aq) + 2 Fe^3+(aq) CI_2(g) + 2 e^- righrarrow 2 CI^-(aq) E degree = +1.36 V Fe^3+(aq) + 3 e^- rightarrow Fe(s) E degree = -0.04 V A) +1.40 V B) -1.32 V C) +1.32 V D) +4.16 V E) -1.40 V Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 degree C. Sn(s)|Sn^2+(aq) 1.8 M) ||Ag^+(aq, 0.055 M)| Ag(s) A) -0.85 V B) -0.94 V C) +0.86 V D) +1.02 V E) +0.98 V
Irving HeathcoteLv2
12 Sep 2019